For ThF4 ksp= 5.0x10^-29. What is the solubility of the sale in water? Show all work
ThF4----> Th+4 + 4F-
Ksp = [ Th+4] {F-]4
Let [Th+4 ] =x hence [F-] =4x
5*10-29= x(4x)4= 256x5
x5= 5*10-29/ 256
x5= 1.95*10-31
x= 7.21*10-7M
For ThF4 ksp= 5.0x10^-29. What is the solubility of the sale in water? Show all work
1. what is the solubility of AgBr with a Ksp of 5.0x10-13 in 0.1M NaBr? Did you expect this to be higher or lower than the solubility of AgBr by itself? 2. Would you expect the solubility of AgBr to be significantly pH dependent? why or why not? 3. The Ksp of Mg(OH)2 is 1.8x10-11 at 25C. What is the pH of a saturated solution of Mg(OH)2 at 25C? 4. Would Mg(OH)2 be more soluble in water or a solution...
please show all work
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Fill in the blanks and Show all work
Identity of SrC2O4 salt :_________
Solubility :__________
Ksp from Solubility (show calculation )
Also answer the Question on the bottom of page 126
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Determine the molar solubility and value of Ksp for each compound in water at 25°C. Include the chemical equation for each equilibrium, the expression for Ksp (in terms of molarities and x), and show all work in calculations Compound 1: SrSO4 Compound 2: Ag2SO4 Chemical equation: Molar solubility (x) = Ksp =
Calculating Molar Solubility:
(Please show all work! will upvote.)
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1)Use the virtual lab to determine the solubility product (Ksp)
for the following solids. Show all work for credit. *should be able
to use the lab to determine the ion concentrations at equilibrium
and use these for the formulas for KSP and then the KSP'S for
solubility. The lab is just to help you get the ion concentration
(a). AgCl (b). SrSO4 (c). Ag2CO3 (d). Sr(IO3)2
2) What is the solubility of the solids listed in question 1, in
moles/liter?...
2)Use the virtual lab to determine the solubility product (Ksp) for the following solids. Show all work for credit. *should be able to use the lab to determine the ion concentrations at equilibrium and use these for the formulas for KSP and then the KSP'S for solubility. The lab is just to help you get the ion concentration (a). AgCl (b). SrSO4 (c). Ag2CO3 (d). Sr(IO3)2 3) What is the solubility of the solids listed in question 2, in moles/liter?...
The solubility of Li3PO4 in water is 0.034 g per 100 mL. What is the solubility product for this salt? (Ksp = [Li]3[PO4]). Please show your work. Thank you!
what is the molar solubility of PbI2 in water. ksp= 1.4x10^-8